Metallic bonding is between metal ions in a sea of delocalised electrons. In Aluminum, there are more delocalised electrons and the ions have a higher charge than Sodium. There is a greater force of attraction between the electrons of aluminum because the protons that are pulling on a 3+ ion are stronger than a 1+ ion. Since it requires more force to overcome these forces of attraction, Aluminum has the higher melting point.
- Troy Moss
Aluminum oxide has a higher melting point than sodium chloride. Aluminum oxide has a melting point of around 2072°C, while sodium chloride has a melting point of 801°C.
The melting point increases from sodium to aluminum because as you move across the periodic table from left to right, the atomic size decreases while the nuclear charge increases. This results in stronger metallic bonding, requiring more energy to overcome and leading to higher melting points. Additionally, aluminum forms metallic bonds that are stronger than those of sodium due to its higher charge and smaller size.
Sodium Chloride has a higher melting point because at room temperature it is a solid but Ethyl alcohol has already melted, as it is liquid.
NaI has ions and has strong electrostatic force of attraction, hence high melting point. Naphthalene has weak van der Waals forces of attraction between the molecules and hence have low melting point.
The melting point of sodium is 97.8 Celsius.
Aluminum oxide has a higher melting point than sodium chloride. Aluminum oxide has a melting point of around 2072°C, while sodium chloride has a melting point of 801°C.
The melting point of sodium chloride is 801 0C. The melting point of aluminium oxide is 2 072 0C.
Yes, sodium has a higher melting point than potassium. Sodium has a melting point of 97.8°C while potassium's melting point is much lower at 63.38°C.
Aluminum oxide would have a higher melting point than sodium chloride. This is because aluminum oxide has stronger bonds between its ions, resulting in a higher energy requirement to break these bonds compared to the weaker bonds in sodium chloride.
Sodium has a melting point of 97.72 oC and rubidium has a melting point of 39.48 oC.
Aluminum oxide (Al2O3) would have a higher melting point than sodium bromide (NaBr). This is because aluminum and oxygen ions in Al2O3 are more strongly bonded through covalent bonds, while sodium and bromide ions in NaBr are held together by weaker ionic bonds. Stronger bonding requires more energy to break, resulting in a higher melting point.
The melting point of cesium is lower than that of sodium. Cesium has a melting point of 28.4°C, while sodium has a melting point of 97.8°C.
The melting point of sodium chloride is 801 0C. The melting point of phosphorus trichloride is -93,6 0C.
Common table salt (sodium chloride) has a much higher melting point than either sodium or chlorine.
The melting point increases from sodium to aluminum because as you move across the periodic table from left to right, the atomic size decreases while the nuclear charge increases. This results in stronger metallic bonding, requiring more energy to overcome and leading to higher melting points. Additionally, aluminum forms metallic bonds that are stronger than those of sodium due to its higher charge and smaller size.
Sodium Chloride has a higher melting point because at room temperature it is a solid but Ethyl alcohol has already melted, as it is liquid.
The higher melting point of sodium fluoride compared to sodium iodide is due to stronger forces of attraction between the ions in the crystal lattice of the fluoride compound. Fluoride ions are smaller and have a higher charge density compared to iodide ions, leading to stronger electrostatic forces between the ions in sodium fluoride, resulting in a higher melting point.